contains TWO pages. [Supplied Data: R = 8.314 J mor1 ~ 1 ; 1 Faraday= 96‚500 C mol-1] Ql. (a) For air at temperatures near 25°C and pressure in the range of 0 bar to 50 bar‚ the JouleThomson coefficient (;J.JT) can be considered as 0.2 K bar- 1• Estimate the final temperature of air if 58 g of air at 25°C and 50 bar undergoes Joule-Thomson throttling to a final pressure of I bar. [2] (b) Calculate ~G for isothermal compression of 30.0 g of water from 1.0 bar to 100.0 bar at 25°C. Consider Vis
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mL when the pressure is 1.00 atm. At the same temperature‚ what is the pressure at which the volume of the gas is 2.0 L? a. | 0.5 atm | c. | 0.20 atm | b. | 5.0 atm | d. | 800 atm | ____ 2. The pressure of a sample of helium is 2.0 atm in a 200-mL container. If the container is compressed to 10 mL without changing the temperature‚ what is the new pressure? a. | 200 atm | c. | 100 atm | b. | 0.10 atm | d. | 40. atm | ____ 3. A sample of argon gas at standard pressure occupies 1000
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describe the design‚ fabrication‚ and calibration of a highly compliant artificial skin sensor. The sensor consists of multilayered mircochannels in an elastomer matrix filled with a conductive liquid‚ capable of detecting multiaxis strains and contact pressure. A novel manufacturing method comprised of layered molding and casting processes is demonstrated to fabricate the multilayered soft sensor circuit. Silicone rubber layers with channel patterns‚ cast with 3-D printed molds‚ are bonded to create embedded
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liquid hydrogen‚ –252.87°C (b) the temperature of a room at 20°C. 2. A constant-volume gas thermometer is calibrated in dry ice (–80.0°C) and in boiling ethyl alcohol (78.0°C). The respective pressures are 0.900 atm and 1.635 atm. (a) What value of absolute zero does the calibration yield? (b) What pressures would be found at the freezing and boiling points of water? (Note that we have the linear relationship P = A + BTc‚ where A and B are constants.) 3. The melting point of gold is 1 064°C‚ and
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|Use for 8-9 |A certain quantity of an ideal gas initially at temperature T0‚ pressure p0‚ and volume V0 is
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100kPa and in the room temperature. This equation shows the product of the pressure(P) and volume(V) equals to the product of the number of moles(n)‚ ideal gas constant (R‚ 8.31451J/molK)‚ and the temperature in Kelvin(T). In order to calculate ‘n’‚ several assumptions must be made. As the substance goes through the boiling water bath‚ the beaker is assumed to only contain the vaporized from of the
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3 (Process variable Review) PRESSURE CONVERSION TABLE mH2O mH2O psi inHg mmHg mbar Pa 1 0.70307 0.34532 0.01359 0.01019 0.000102 psi 1.42233 1 0.49115 0.01934 0.0145 0.00015 What is the absolute pressure equivalent to 150 psi_g in psi_a? inHg 2.8959 2.03602 1 0.03937 0.02953 0.000295 mmHg 73.55592 51.71493 25.4 1 0.75006 0.0075 mbar 98.0665 68.9476 33.8639 1.3332 1 0.01 Pa 9806.65 6894.757 3386.388 133.322 100 1 (Ans. 164.7 psi-a) What is the vacuum pressure equivalent to 4.3 psia in psi
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possible. • It is applicable to actual gases at low density. • At low pressure and high temperature‚ the density of gas d d it f decreases and gas b h d behaves as an ideal gas under these conditions Non-Ideal or Real Gas •Low Temperature •High P Hi h Pressure •Particle size significant compared to space between particles ti l Interactions •Interactions between particles are significant Ideal Gas Equation of State • At low pressure and high temperature the temperature‚ density of gas decreases
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for each gas are in 1atm. 5. Even though the number of molecules in 1 atm of gas at constant pressure and temperature is identical‚ the number of atoms in the gas at STP can vary depending on the gas. How many atoms are there in one mole of methane (CH4) 1 mole of Methane CH4 = (6.022 x 1023 atoms/mole) = 6.022x1023 atoms of Methane in one mole 6. In this experiment‚ the pressure (P) was 1 atm‚ the temperature (T) was 295 K‚ the volume (V) was 0.150 L‚ and the number of moles (n)was
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energy is required to overcome these attractive forces since the molecules are relatively small. Therefore‚ the liquid vaporizes easily and quickly at temperatures less than 100°C. While the substance is in the vapor phase‚ you can measure its volume‚ pressure‚ and temperature. You can then use the ideal gas law to calculate the number of moles of the substance. Finally‚ you can use the number of moles of the gas to calculate molar mass. OBJECTIVES In this experiment‚ you will • Evaporate a sample
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